Start Discovering Solved Questions and Your Course Assignments
TextBooks Included
Active Tutors
Asked Questions
Answered Questions
One approach is to first find the total weight of your sample container and its contents, pour or shake some of this material out into a labelled beaker.
This experiment involves a number of redox reactions. They are carried out in the following order of stages.
A 25.00 mL portion of a solution known to contain NaBr was treated with excess AgNO3 to precipitate 0.02578 g of AgBr.
A solution containing 100.0 mL of 0.150 M HCl is titrated with 75.0 mL of 0.300 NaOH. What is the pH of the resulting solution?
What is the average mass of calcium in each sample? Assume that the relative uncertainties in atomic mass are small compared the uncertainty of the total mass.
What are the major differences and similarities between these two specra. Which is more useful for quantitative work? and which is for qualitative?
An explanation of the splitting pattern observed with a discussion of splitting constants for non-equivalent protons.
A solid samples are prepared by examination by IR spectroscopy by fusing them in a KBr pellet or dissolving them in CCl4 and subtracting.
Would the IR spectrum of polymer polystyrene have sharp or broad signals? Explain.
A mass spectrometer is a device that uses a magnetic field to sort atoms by mass. In this device, atoms whose masses are to be determined.
Mass spectrometry (MS) makes use of the motion of ions in electric and magnetic fields in order to sort them according to their mass-to-charge ratios.
Describe the Factors influencing the sensitivity of the elements being measured and potential use of ICP-MS besides total elemental analysis.
How many parent ion peaks do you expect in the mass spectrum of the Cl2+ ion?
Xenon is a monatomic element. Therefore, no fragmentation occurs and the peaks in the mass spectrum are solely attributable to xenon ions.
Add 25 mL HCl (of unknown concentration) to the flask. Add 2 drops of phenolphthalein to the flask. Fill a burette with 50 mL of 1M NaOH solution.
Outline a titration procedure for determining the exact concentration of the aqueous nitric acid.
A sample of 0.0054 mol propanoic acid was dissolved in water to give 50ml solution. This solution is titrated with 0.150 M of NaOH.
What's the pH at the first equivalence point of 0.100M of malonic acid of 25mL with 0.140M of NaOH? What's the pH after 25mL of NaOH were added?
In a titration reaction using sodium hydroxide and KHP, which substance is the proton donor and which is the proton acceptor?
Calculate the pH at 0, 10.0, 25.0, 50.0, and 60.0 mL of titrant in the titration of 50.0 mL of 0.100 M NH3 with 0.100 M HCl.
A 25.0 ml sample of an aqueous solution of pure benzoic acid is titrated using standardized 0.150 M NaOH
A 30 mL sample of 0.35 M of lactic acid is titrated with a 0.25 M NaOH solution. Calculate the pH before NaOH is added.
The 125 mL flask can be wet when the 25 mL of seawater is added using the volumetric pipet. Why doesn't the water in the flask cause problems in the calculation
If potassium permanganate had been used as the titrant instead of cerium(IV), what would the balanced overall reaction be?
Using the following pKb (pKb = 4.11) of an unknown base, calculate the Ka of the corresponding conjugate acid